AP Chemistry Chapter 10 and 11 Jeopardy

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AP ChemistryChapter 10 and 11 Jeopardy

• Jennie L. Borders

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Round 1 Chapter 10
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Gas Laws Ideal Gas Law Molar Mass Effusion/ Diffusion Partial Pressures Kinetic Molecular Theory
100 100 100 100 100 100
200 200 200 200 200 200
300 300 300 300 300 300
400 400 400 400 400 400
500 500 500 500 500 500
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Round 2 Chapter 11

• Click to go to Round 2

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Gas Laws 100

• A sample of a gas (5.0mol) at 1.0 atm is expanded
  at constant temperature from 10L to 15L. What is
  the final pressure in atm?

0.67 atm
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Gas Laws 200

• A balloon originally had a volume of 4.39L at
  44oC and a pressure of 729 torr. The balloon must
  be cooled to what Celsius temperature in order to
  reduce its volume to 3.78L (at constant pressure).

-0.05oC
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Gas Laws 300

• A sample of He gas (2.35 mol) occupies 57.9L at
  300K and 1 atm. What is the volume of this sample
  at 423K and 1 atm?

81.64L
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Gas Laws 400

• A sample of an ideal gas (3L) in a closed
  container at 25oC and 76 torr is heated to 300oC.
  What is the pressure in torr now?

146.13 torr
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Gas Laws 500

• A closed-end manometer was attached to a vessel
  containing argon. The difference in the mercury
  levels in the two arms of the manometer was
  12.2cm. Atmospheric pressure was 783mm Hg. What
  is the pressure of argon in the container in mm
  Hg?

122mm Hg
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Ideal Gas Law 100

• What is the pressure in kPa exerted by 1.3 mol of
  gas in a 13L flask at 22oC?

245.15 kPa
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Ideal Gas Law 200

• How many moles of gas are contained in a 0.325L
  flask at 0.914 atm and 19oC?

0.012 mol
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Ideal Gas Law 300

• The density of ammonia gas in a 4.32L container
  at 837 torr and 45oC is ___ g/L.

0.714 g/L
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Ideal Gas Law 400

• A sample of gas (1.9 mol) is in a flask at 21oC
  and 697 mm Hg. The flask is opened and more gas
  is added to the flask. The new pressure is 795 mm
  Hg and the temperature is now 26oC. How many
  moles of gas are left in the flask?

2.13 mol
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Ideal Gas Law 500

• What volume in mL of sulfur dioxide can be
  produced by the complete reaction of 3.82g of
  calcium sulfite with excess HCl, when the final
  pressure is 827 torr at 44oC?

760 mL SO2
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Molar Mass 100

• What is the molar mass of 3.5g of a gas that
  occupies 2.1L at STP?

37.23 g/mol
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Molar Mass 200

• What is the molar mass of a gas that has a
  density of 6.7 g/L at STP?

150.08 g/mol
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Molar Mass 300

• What is the molar mass of a gas that has a
  density of 7.10 g/L at 25oC and 1 atm?

173.74 g/mol
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Molar Mass 400

• What is the molar mass of a gas that has a
  density of 5.75 g/L at STP?

128.86 g/mol
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Molar Mass 500

• What is the molar mass of air at STP if it has a
  density of 1.285 g/L?

28.78 g/mol
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Effusion/Diffusion 100

• At 333K, which of the following pairs of gases
  would have the most nearly identical rates of
  effusion?
• a. N2O and NO2
• b. CO and N2
• c. N2 and O2
• d. CO and CO2
• e. NO2 and N2O4

b. CO and N2
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Effusion/Diffusion 200

• Of the following gases, which one would have the
  greatest rate of effusion at a given temperature?
• a. NH3
• b. CH4
• c. Ar
• d. HBr
• e. HCl

b. CH4
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Effusion/Diffusion 300

• Arrange the following gases in order of
  increasing average molecular speed at 25oC.
• He, O2, CO2, N2

CO2, O2, N2, He
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Effusion/Diffusion 400

• A tank containing both HF and HBr gases developed
  a leak. The ratio of the rate of effusion of HF
  to HBr is ___.

2

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Effusion/Diffusion 500

• A sample of oxygen gas was found to effuse at a
  rate equal to three times that of an unknown gas.
  What is the molar mass of the unknown gas?

288 g/mol
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Partial Pressures 100

• A gas mixture of Ne and Ar has a total pressure
  of 4.00 atm and contains 16 mol of gas. If the
  partial pressure of N2 is 2.75 atm, how many
  moles of Ar are in the mixture?

4.96 mol Ar
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Partial Pressures 200

• A mixture of He and Ne at a total pressure of
  0.95 atm is found to contain 0.32 mol of He and
  0.56 mol of Ne. What is the partial pressure of
  Ne in atm?

0.61 atm
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Partial Pressures 300

• In a gas mixture of He, Ne, and Ar with a total
  pressure of 8.40 atm, the mole fraction of Ar is
  ___ if the partial pressures of He and Ne are
  1.50 and 2.00 atm, respectively.

0.58
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Partial Pressures 400

• A sample of NaH weighing __g will produce 982mL
  of gas at 28oC and 765 torr, when the hydrogen is
  collected over water. The vapor pressure of water
  at this temperature is 28 torr.
• NaH H2O ? NaOH H2

0.936g NaH
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Partial Pressures 500

• In an experiment, 225mL of wet H2 is collected
  over water at 27oC and a barometric pressure of
  748 torr. How many grams of Zn have been
  consumed? The vapor pressure of water at 27oC is
  26.74 torr.
• Zn H2SO4 ? ZnSO4 H2

0.57g Zn
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Kinetic Molecular Theory 100

• Which of the following is NOT part of the
  kinetic-molecular theory?
• a. Atoms are neither created nor destroyed by
  ordinary chemical reactions.
• b. Attractive and repulsive forces between gas
  molecules are negligible.
• c. Gases consist of molecules in continuous,
  random motion.
• d. Collisions between gas molecules do not result
  in the loss of energy.
• e. The volume occupied by all of the gas
  molecules in a container is negligible compared
  to the volume of the container.

a. Atoms are neither created nor destroyed by
ordinary chemical reactions.
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Kinetic Molecular Theory 200

• An ideal gas differs from a real gas in that the
  molecules of an ideal gas have no _____ and no
  _____.

volume, attractions
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Kinetic Molecular Theory 300

• A real gas will behave most like an ideal gas
  under condition of ________.

high temperature and low pressure
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Kinetic Molecular Theory 400

• The kinetic molecular theory predicts that
  pressure rises as the temperature of a gas
  increases because _______.

As temperature rises, kinetic energy rises
resulting in more collisions with the wall of the
container and harder collisions with the wall.
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Kinetic Molecular Theory 500

• According to the kinetic-molecular theory, if the
  temperature of a gas is raised from 100oC to
  200oC, the average kinetic energy of the gas will
  ______.

Increase by a factor of 1.27
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Vocabulary Intermolecular Forces Boiling Point Heating Curve Phase Diagram Solids
200 200 200 200 200 200
400 400 400 400 400 400
600 600 600 600 600 600
800 800 800 800 800 800
1000 1000 1000 1000 1000 1000
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Vocabulary 200

• What is equilibrium?

When two opposite processes are occurring at the
same rate.
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Vocabulary 400

• What is viscosity?

The resistance of a liquid to flow.
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Vocabulary 600

• What is surface tension?

The amount of energy needed to increase the
surface area.
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Vocabulary 800

• What is capillary action? What types of forces
  encourage and discourage capillary action?

Capillary action is the process of a liquid
climbing up a narrow tube. Adhesive forces
encourage capillary action and cohesive forces
discourage capillary action.
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Vocabulary 1000

• What is critical temperature and critical
  pressure?

Critical temperature is the highest temperature
at which pressure can still convert a gas into a
liquid. Critical pressure is the pressure needed
to convert a gas to a liquid at critical
temperature.
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Intermolecular Forces 200

• Of the following substance, which experiences
  ONLY London dispersion forces?
• CH3OH, NH3, H2S, CH4, HCl

CH4
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Intermolecular Forces 400

• What intermolecular forces are present when NaCl
  dissolves in H2O?

Ion-dipole forces between ions and water.
Hydrogen bonding and dipole attractions between
water molecules. Dipersion forces between all
molecules.
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Intermolecular Forces 600

• What intermolecular forces are present in C12H26
  molecules?

London Dispersion Forces
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Intermolecular Forces 800

• Which one of the following exhibits dipole-dipole
  attractions?
• XeF4, AsH3, CO2, BCl3, Cl2

AsH3
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Intermolecular Forces 1000

• In which of the following molecules is hydrogen
  bonding likely the most significant component of
  the total intermolecular forces?
• CH4, C5H11OH, C6H13NH2, CH3OH, CO2

CH3OH
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Boiling Point 200

• What is vapor pressure?

Vapor pressure is the pressure of a vapor above
its liquid.
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Boiling Point 400

• Which of the following has the highest boiling
  point?
• H2O, CO2, CH4, Kr, NH3

H2O
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Boiling Point 600

• Which of the following has the highest boiling
  point?
• N2, Br2, H2, Cl2, O2

Br2
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Boiling Point 800

• Which of the following would have the lowest
  boiling point?
• PH3, H2S, HCl, SiH4, H2O

SiH4
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Boiling Point 1000

• Which of the following has the highest melting
  point?
• S8, I2, SiO2, SO2, C6H6

SiO2 (network solid)
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Heating Curve 200

• What is a supercooled liquid?

A supercooled liquid is a liquid that has been
cooled below the freezing point without being
converted to a solid.
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Heating Curve 400

• What does 2 represent? What formula do we use at
  2?

Melting DHfus
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Heating Curve 600

• What does 5 represent? What formula do we use at
  5?

Gas q mcDT
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Heating Curve 800

• What is the change in enthalpy when 1.00 mol of
  ice at -50.0oC to water at 70.0oC?
• cice 2.09 J/gK, cH2O 4.18 J/gK, csteam 1.84
  J/gK, DHfus 6.01 kJ/mol, DHvap 40.67 kJ/mol

13158J
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Heating Curve 1000

• What is the change in enthalpy when 25.0g of ice
  at -4oC to steam at 110oC?
• cice 2.09 J/gK, cH2O 4.18 J/gK, csteam 1.84
  J/gK, DHfus 6.01 kJ/mol, DHvap 40.67 kJ/mol

76042J
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Phase Diagram 200

• On the phase diagram, which letter corresponds to
  the critical temperature and critical pressure?

D
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Phase Diagram 400

• One the phase diagram, which letter corresponds
  to the gas and solid phases at equilibrium?

C
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Phase Diagram 600

• On the phase diagram, which letter corresponds to
  the solid phase?

A
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Phase Diagram 800

• On the phase diagram, which state of matter is
  the substance at 25oC and 1 atm?

liquid
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Phase Diagram 1000

• Which of the following statements is always true
  about a phase diagram?
• a. The slope between the liquid and solid phases
  is negative.
• b. The slope between the liquid and solid phases
  is positive.
• c. The slope between the vapor and liquid phases
  is positive.
• d. The pressure at the triple point is greater
  than 1 atm.

c. The slope between the vapor and liquid phases
is positive.
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Solids 200

• What is the difference in a crystalline solid and
  an amorphous solid?

Crystals have an orderly repeating 3-D structure.
Amorphous solids have a random structure.
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Solids 400

• _____ solids consist of atoms or molecules held
  together by dipole forces, dispersion forces,
  and/or hydrogen bonds.

Molecular
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Solids 600

• What fraction of the volume of each corner atom
  is actually within the volume of a face-centered
  cubic unit cell?

1/8
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Solids 800

• CsCl crystallizes in a unit cell that contains a
  Cs ion at the center of a cube and Cl- ions at
  each corner. The unit cell of CsCl is ________.

Body-centered cubic
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Solids 1000

• CsCl crystallizes in a unit cell that contains
  the Cs ion at the center of a cube that has Cl-
  at each corner. How many Cs and Cl- ions are in
  the unit cell?

1Cs and 1Cl-